The maximum mass of anhydrous zinc chloride that could be obtained from the products of the reaction is 8.18 g
<h3>Stoichiometry </h3>
From the question, we are to determine the maximum mass of anhydrous zinc chloride that could be obtained
From the given balanced chemical equation,
ZnO + 2HCl → ZnCl₂ + H₂O
This means 1 mole of ZnO will completely react with 2 moles of HCl to produce 1 mole of ZnCl₂ and 1 mole of H₂O
From the given information
Number of moles of ZnO = 0.0830 mole
Now, we will calculate the number of moles of HCl that is present
Volume of HCl added = 100 cm³ = 0.1 dm³
Concentration of the HCl = 1.20 mol/dm³
Using the formula,
Number of moles = Concentration × Volume
Number of moles of HCl present = 1.20 × 0.1 = 0.120 mole
Since
1 mole of ZnO will completely react with 2 moles of HCl to produce 1 mole of ZnCl₂
Then,
0.06 mole of ZnO will react with the 0.120 mole of HCl to produce 0.06 mole of ZnCl₂
Therefore, maximum number of moles of anhydrous zinc chloride that could be produced is 0.06 mole
Now, for the maximum mass that could be produced
Using the formula,
Mass = Number of moles × Molar mass
Molar mass of ZnCl₂ = 136.286 g/mol
Then,
Mass = 0.06 × 136.286
Mass = 8.17716 g
Mass ≅ 8.18 g
Hence, the maximum mass of anhydrous zinc chloride that could be obtained from the products of the reaction is 8.18 g
Learn more on Stoichiometry here: brainly.com/question/11910892
